Method for preparing complex oxide and complex oxide prepared thereby

ABSTRACT

Ba(OH) 2 .8H 2 O is fused by heating. The fused Ba(OH) 2  is allowed to react with TiO 2  powder having a specific surface area of 250 m 2 /g or more to prepare a cubic crystalline BaTiO 3  having high crystallinity. The BaTiO 3  is calcined to yield a fine, tetragonal crystalline BaTiO 3  powder having high crystallinity. Thus, a high quality BaTiO 3  having high crystallinity can be prepared at a low cost.

BACKGROUND OF THE INVENTION

[0001] 1. Field of the Invention

[0002] The present invention relates to methods for manufacturing a complex oxide powder and complex oxide powders, and particularly to a method for manufacturing a complex oxide powder used for electronic materials, such as dielectric ceramics, and a complex oxide powder prepared by the method.

[0003] 2. Description of the Related Art

[0004] Monolithic capacitors have recently been miniaturized with their capacitance becoming larger, and accordingly, the thickness of dielectric elements has become smaller. In order to manufacture such a laminated monolithic capacitor, the crystal grains of dielectric ceramics need to be small and the crystal growth of the grains must be suppressed. Accordingly, complex oxides constituting the ceramics are required to have a small grain size and high crystallinity.

[0005] Barium titanate (BaTiO₃) powder has been typically used as such a complex boxide, and a wet synthesis (Kubo, K. et al., “Wet process for synthesizing barium titanate”, Journal of Chemical Industry by The Chemical Society of Japan, Vol. 71, No. 1, 114-118 (1968)) is widely known as a method for preparing BaTiO₃ powder.

[0006] In this method, barium hydroxide octahydrate (Ba(OH)₂.8H₂O) and a titanium oxide (TiO₂) gel containing about 95% of water are mechanically triturated and mixed to react with each other while carbon dioxide is removed. The resulting precipitate is separated from the reaction product. Then, acetic acid (6 N) is added to the precipitate, followed by heating to 50° C. Unreacted Ba(OH)₂ and the by-products BaCO₃ and Ba₂TiO₄ are dissolved and extracted. The remaining precipitate is washed with water and dried to yield the BaTiO₃.

[0007] As for another method, a hydrolysis method is disclosed in Japanese Examined Patent Application Publication No. 3-39014. In this method, a product from hydrolysis of a titanium compound and a water-soluble barium salt are allowed to react with each other in a strong alkaline aqueous solution to yield BaTiO₃ fine particles. Specifically, this publication describes creating a product from the hydrolysis of a titanium compound, such as TiCl₄, and Ba(NO₃)₂, in a strong alkaline aqueous solution, such as KOH or NaOH of pH 13.0 or more, to yield cubic crystalline BaTiO₃.

[0008] A pulverization method, hydrothermal synthesis, sol-gel method, and alkoxidehydroxide route are also known as methods for preparing BaTiO₃ powder.

[0009] The pulverization method is suitable for preparing a fine particle material at a low cost. In the pulverization method, a mixture of BaCO₃ and TiO₂ is mechanically pulverized and uniformly mixed using a ball mill, a sand mill, or the like. The resulting fine particles are dried and calcined to yield the BaTiO₃ powder.

[0010] In the hydrothermal synthesis, an active titanium entity ([Ti(OH)₆]²⁻) having a number of hydroxyl groups and a large specific surface area is prepared, in advance, by hydrolysis of TiCl₄ or titanium alkoxide. This active titanium entity is heated under a high pressure with Ba(OH)₂ in an autoclave so that barium ions (Ba²⁺) diffuse into TiO₂ to synthesize the BaTiO₃.

[0011] In the sol-gel method, a titanium compound is allowed to directly react with a barium compound. A mixed solution of titanium alkoxide and barium alkoxide may used as a starting material, or a solution of an alkoxide precursor including titanium and barium at a ratio derived from the stoichiometry may be used as the starting material.

[0012] In the alkoxide-hydroxide route, titanium alkoxide is hydrolyzed in a solution containing Ba²⁺ to yield BaTiO₃. When titanium alkoxide is hydrolyzed in a Ba(OH)₂ solution, the alkoxide solution becomes clouded immediately. Specifically, TiO₂ (or [Ti(OH)₆]²⁻) is first produced in the Ba(OH)₂ solution, and then the TiO₂ (or [Ti(OH)₆]²⁻) reacts with Ba²⁺. Thus, by diffusing the Ba²⁺ into the TiO₂, as in the hydrothermal synthesis, BaTiO₃ is prepared.

[0013] However, the wet synthesis needs to separate unreacted Ba(OH)₂ from the precipitate, and also to extract by-produced BaCO₃ and Ba₂TiO₄ by dissolution to separate them from the BaTiO₃. Thus, the wet synthesis is complicated. In addition, the resulting BaTiO₃ is likely to contain Ba₂TiO₄, and thus the BaTiO₃ crystals could be imperfect.

[0014] Also, since the concentration of TiO₂ is low due to the use of TiO₂ containing 95% water, the reaction between TiO₂ and Ba(OH)₂ does not efficiently proceed.

[0015] Furthermore, since the dissolution is performed with an acid, such as acetic acid, the resulting crystals are likely to be damaged, or Ba²⁺ could be eluted to vary the mole fractions of the BaTiO₃.

[0016] In the hydrolysis method, an alkali metal, such as K or Na, is likely to adhere to the resulting BaTiO₃ because the reaction of a product from hydrolysis of a titanium compound with a water-soluble barium salt is conducted in a strong alkaline aqueous solution of pH 13.0 or more. As a result, impurities which cause failure in insulation resistance remain in BaTiO₃ in several hundreds of ppm even if the resulting BaTiO₃ is washed. Therefore, such BaTiO₃ is not suitable for a dielectric ceramic material which needs to be laminated.

[0017] In the pulverization method, zirconia or the like contained in pulverizing media of the ball mill or the like could be mixed into BaTiO₃. Thus, it is difficult to prepare a pure BaTiO₃ powder. Also, since BaCO₃ and TiO₂ pulverized in this method have a relatively large particle size, the degree of pulverization is limited. Specifically, these materials have extensive particle size distributions and their particles do not grow uniformly. It is therefore difficult to make the resulting ceramic particle size small and uniform.

[0018] The hydrothermal synthesis requires large equipment and batch processes, and consequently, workability and manufacturing efficiency are degraded. Thus, the hydrothermal synthesis limits the ability to effect cost reduction and increases costs.

[0019] In the sol-gel method, cubic crystalline BaTiO₃ can be obtained by calcination at about 400° C. However, this method must be performed in a dry atmosphere because barium alkoxide is liable to react with water violently in the atmosphere to emit smoke. Also, the alkoxides used as the starting material are undesirably expensive.

[0020] In the alkoxide-hydroxide route, titanium alkoxide is dissolved in Ba(OH)₂ to synthesize barium titanate. However, in order to complete this reaction, an excessive amount of Ba(OH)₂ is required, or NaOH or KOH must be added.

[0021] If Ba(OH)₂ is used excessively, Ba²⁺ remains in the solution after the reaction, thus making it difficult to control the composition of BaTiO₃. Also, equipment for recovering barium is necessary.

[0022] If NaOH or KOH is added, Na⁺ or K⁺ remains in the solution after the reaction, thus interfusing into the resulting BaTiO₃ to act as an impurity. Thus, it is difficult to prepare pure BaTiO₃.

[0023] Furthermore, since hydrolysis of an alkoxide by-produces an alcohol which is a hazardous organic solvent, explosion proof equipment is needed, increasing costs.

SUMMARY OF THE INVENTION

[0024] Accordingly, the object of the present invention is to provide a method for manufacturing a high-quality complex oxide fine particle powder, such as barium titanate powder, having a high crystallinity at a low cost, and to provide a complex oxide powder prepared by the method.

[0025] The inventors of the present invention have conducted intensive research to achieve a fine, highly crystalline barium titanate powder by a simple method. As a result, it has been shown that, by fusing barium hydroxide octahydrate (Ba(OH)₂.8H₂O) by heating, a high concentration of active barium solution can be prepared, and that, by allowing the barium solution to react with titanium oxide (TiO₂) powder, a pure, fine BaTiO₃ powder can be easily prepared. In addition, this method may be applied to other complex oxides similar to BaTiO₃.

[0026] According to an aspect of the present invention, a method is provided for preparing a complex oxide powder having a perovskite structure expressed by the general formula ABO₃. The method includes a fusion step of fusing a hydroxide of an element constituting the A site of the general formula ABO₃ by heating. The hydroxide contains crystal water. The method also includes a reaction step of allowing the fused hydroxide to react with an oxide powder of an element constituting the B site of the general formula ABO₃ to yield a reaction product. The oxide powder of the B site element comprises specific ultrafine particles.

[0027] When the complex oxide powder is BaTiO₃, Ba(OH)₂.8H₂O may be used as the hydroxide and TiO₂ powder may be used as the ultrafine oxide powder.

[0028] In other words, the hydroxide may be Ba(OH)₂.8H₂O in the method of the present invention and the oxide powder of the B site element may be TiO₂ powder. Thus, a desired BaTiO₃ powder can be prepared at a low cost.

[0029] Instead of a hydroxide containing crystal water, an anhydrous hydroxide containing an amount of water equivalent to the amount of the crystal water can be used.

[0030] Accordingly, the present invention is also directed to a method for preparing a complex oxide powder having a perovskite structure expressed by the general formula ABO₃. The method includes a dissolution step of dissolving an anhydrous hydroxide of an element constituting the A site of the general formula ABO₃ in a predetermined amount of water. The method also includes a reaction step of allowing the dissolved hydroxide to react with an oxide powder of an element constituting the B site of the general formula ABO₃ to yield a reaction product. The oxide powder of the B site element comprises specific ultrafine particles. The amount of water may be equivalent to the amount of crystal water contained in a hydrous hydroxide of the element constituting the A site.

[0031] When the complex oxide powder is BaTiO₃, Ba(OH)₂ may be used as the hydroxide and TiO₂ powder may be used as the ultrafine oxide powder.

[0032] In other words, the anhydrous hydroxide may be Ba(OH)₂ in the method of the present invention and the oxide powder of the B site element may be TiO₂ powder. Thus, a desired BaTiO₃ powder can be prepared at a low cost.

[0033] In order to prepare an ultrafine final product, or the complex oxide, having high crystallinity, the oxide powder used as a material must be ultrafine and highly crystalline.

[0034] Preferably, the ultrafine specific particles have a specific surface area of about 250 m²/g or more.

[0035] By using an oxide powder having a specific surface area of about 250 m²/g or more, the formation of heterogeneous phases can be as suppressed as much as possible. Thus, an ultrafine, highly crystalline complex oxide powder can be prepared.

[0036] Preferably, the hydroxide and the oxide powder are weighed such that the mole ratio of the A site element A to the B site element B is in the range of about 0.990 to 1.010. Thus, a pure complex oxide powder not containing impurities can be prepared.

[0037] The reaction step may be performed under atmospheric pressure. Thus, a desired complex oxide powder can be prepared at a low cost without using special large equipment.

[0038] Preferably, the reaction step comprises a substep of applying ultrasonic waves. Preferably, the reaction product has a specific surface area in the range of about 60 to 100 m²/g.

[0039] By applying ultrasonic waves, a much finer reaction product having a specific surface area of about 60 to 100 m²/g can be prepared before calcination.

[0040] The method may further include a calcination step of calcining the reaction product.

[0041] By calcining the reaction product, an ultrafine, highly crystalline complex oxide powder can be prepared.

[0042] The method may further include a dispersion step of dispersing the reaction product in a liquid and a calcination step of calcining the dispersed reaction product.

[0043] By dispersing the reaction product in a liquid and then calcining the dispersed product, the crystallographic axial ratio c/a can be further increased.

BRIEF DESCRIPTION OF THE DRAWINGS

[0044]FIG. 1 is a block flow diagram of a method for preparing a complex oxide powder according to an embodiment of the present invention;

[0045]FIG. 2 is an illustration showing a reaction path of BaTiO₃ synthesis of the present invention;

[0046]FIG. 3 is an illustration showing another reaction path of BaTiO₃ synthesis of the present invention;

[0047]FIG. 4 is a transmission electron micrograph of crystals after 5 minutes have elapsed from the start of a reaction in a reaction step of synthesizing BaTiO₃;

[0048]FIG. 5 is a transmission electron micrograph of crystals after 30 minutes have elapsed from the start of the reaction in the reaction step of synthesizing BaTiO₃;

[0049]FIG. 6 is a transmission electron micrograph of crystals after 60 minutes have elapsed from the start of the reaction in the reaction step of synthesizing BaTiO₃;

[0050]FIG. 7 is a scanning electron micrograph of non-calcined BaTiO₃ (dried at 200° C.);

[0051]FIG. 8 is a scanning electron micrograph of BaTiO₃ calcined at 900° C.;

[0052]FIG. 9 is a scanning electron micrograph of BaTiO₃ calcined at 950° C.;

[0053]FIG. 10 is a scanning electron micrograph of BaTiO₃ calcined at 1000° C.;

[0054]FIG. 11 is an X-ray diffraction diagram resulting from Experiment 2;

[0055]FIG. 12 is a graph showing the relationships between the particle size and the axial ratio c/a of BaTiO₃ powders of an Example and a comparative example;

[0056]FIG. 13 is an X-ray diffraction diagram resulting from Experiment 3; and

[0057]FIG. 14 is an X-ray diffraction diagram resulting from Experiment 4.

DESCRIPTION OF THE PREFERRED EMBODIMENTS

[0058] In the invention, a hydroxide of an A site element is dissolved in water at a high concentration forming a “fused hydroxide” and the solution is combined with an oxide of a B site element and the reaction allowed to proceed. The water used can be the water of hydration of the hydroxide or an equivalent amount of water when an unhydrated hydroxide is used as a reactant. Because the amount of water generally does not significantly exceed the amount which represents the hydration amount, the A element concentration in the solution is high, e.g., generally about 10 mol % or more. The dissolution generally involves heating at a temperature which does not drive the water out of the system.

[0059] The present invention will now be further illustrated with reference to the drawings.

[0060]FIG. 1 is a block flow diagram showing steps of a method for preparing BaTiO₃ powder, according to an embodiment of the present invention.

[0061] Ba(OH)₂.8H₂O is prepared to act as an hydroxide, containing crystal water, of an element constituting the A site of a perovskite structure expressed by the general formula ABO₃. TiO₂ powder is also prepared to act as an oxide powder, having a specific surface area Sw of about 250 m²/g or more, of an element constituting the B site of ABO₃.

[0062] The reason why the TiO₂ powder having a specific surface area of about 250 m²/g or more is selected is as follows. If a TiO₂ powder having a specific surface area of less than about 250 m²/g is used, heterogeneous phases, such as Ba₂TiO₄ and BaTi₂O₅, are formed before calcination; hence, cubic crystalline BaTiO₃ having high crystallinity cannot be obtained. The final product BaTiO₃ powder is also not tetragonal crystalline even after calcination is performed.

[0063] Accordingly, the TiO₂ powder used in the present invention has a specific surface area of about 250 m²/g or more in order to obtain a tetragonal crystalline BaTiO₃ powder with reliability after calcination.

[0064] The crystals of TiO₂ may have a rutile structure or an anatase structure. However, the rutile structure is likely to allow unreacted TiO₂ to remain, and therefore, an anatase-type TiO₂ is preferable.

[0065] The process of the method will now proceed to a mixing step 1. The mixing step is divided into two steps of a fusion/dissolution step 1a and a reaction step 1b.

[0066] In the fusion/dissolution step 1a, Ba(OH)₂.8H₂O and TiO₂ are weighed such that the mole ratio Ba/Ti of Ba to Ti of BaTiO₃to be synthesized is about 1, and are mixed and heated in a container at a predetermined temperature (for example, at about 60 to 110° C.) to fuse the Ba(OH)₂.8H₂O.

[0067] Since Ba(OH)₂.8H₂O contains crystal water (octahydrate), the fusion of Ba(OH)₂.8H₂O means that the Ba(OH)₂ is dissolved in the crystal water to yield a Ba solution containing a high concentration of activated Ba²⁺. In the reaction step 1b, the Ba solution is allowed to react with the TiO₂ under atmospheric pressure, and thus a reaction product, or BaTiO₃, is produced in a slurry form after a predetermined period of time (for example, after about an hour).

[0068] In other words, the fusion/dissolution step 1a and the reaction step 1b proceed consecutively to produce a BaTiO₃ slurry from the Ba(OH)₂.8H₂O and the TiO₂, as shown in formula (1):

Ba(OH)₂.8H₂O+TiO₂→BaTiO₃+9H₂O   (1)

[0069] It is known that BaTiO₃ is synthesized through the two reaction paths (1) and (2) shown in FIGS. 2 and 3 (J. O. Eckert Jr, et al., J. Am. Ceram. Soc., 79[11], 2929-39, (1996)).

[0070] In reaction path (1), a homogeneous nucleation (a) and a heterogeneous nucleation (b) proceed in parallel to produce BaTiO₃ when TiO₂ is dissolved in the Ba solution. In reaction path (2), Ba is diffuses among TiO₂ particles to produce BaTiO₃.

[0071] Since the solubility of TiO₂ is low and the degree of critical saturation of BaTiO₃ is high, the growth of BaTiO₃ particles becomes extremely slow after the nucleation of BaTiO₃. It is therefore considered that reaction path (1) is predominant to reaction path (2) in an early stage of the reaction, and that reaction path (2) becomes predominant in a later stage.

[0072] However, the TiO₂ powder has a large specific surface area Sw of about 250 m²/g or more, in the method of the present invention so that it can be rapidly dissolved. As a result, a precipitate serving as seed crystals for particle growth is sufficiently supplied and, thus, reaction path (1) substantially completes the synthesis.

[0073] A larger specific surface area of TiO₂ helps the TiO₂ dissolve; hence, as the specific surface of TiO₂ becomes larger, reaction path (1) is more rapidly completed to produce BaTiO₃. The specific surface area of TiO₂ is, therefore, 250 m²/g or more and there is no upper limit.

[0074] In a slurry preparation step 2, the BaTiO₃ reaction product is placed in a sand mill containing pulverizing media, and is pulverized with heating at the above-described predetermined temperature (for example, at about 60 to 110° C.) to prepare a slurry. The slurry is then recovered.

[0075] Then, the slurry was dried in a drying step 3, at a predetermined temperature (for example, at 200° C.) in an oven to prepare a BaTiO₃ powder having an equivalent specific surface diameter of about 20 nm.

[0076] In a following calcination step 4, the resulting BaTiO₃ powder is calcined at a temperature of about 900 to 1000° C. for about 2 hours so that the particles grow to an equivalent specific surface diameter of about 100 to 350 nm. Thus, the crystal system changes to a tetragonal crystal system to yield a highly pure, ultrafine BaTiO₃ powder.

[0077] The resulting BaTiO₃ powder has tetragonal crystals having a crystallographic axial ratio c/a of the c axis to the a axis in the range of about 1.0068 to 1.0092; hence the BaTiO₃ powder does not include heterogeneous phases and is highly crystalline.

[0078] The mole ratio Ba/Ti of Ba constituting A site to Ti constituting the B site is about 0.990 to 1.010 in the BaTiO₃ powder; hence, the BaTiO₃ powder is highly pure.

[0079] In this embodiment, by preparing a high concentration of activated Ba solution, a sufficiently high concentration of hydroxide ions can be obtained. It is therefore not necessary to add an alkali metal element to prepare BaTiO₃ powder.

[0080] The method of the invention does not need to use a hazardous alkoxide or excessive alkali, nor thus, need explosion proof equipment such as that required in the alkoxide-hydroxide route. Also, since the reaction step can be performed at a low temperature of about 60 to 110° C. under atmospheric pressure, the manufacturing cost is reduced, without the necessity of pressure resistant equipment required in hydrothermal synthesis.

[0081] By allowing Ba(OH)₂.8H₂O to react with ultrafine TiO₂ powder while being heated, an ultrafine BaTiO₃ powder containing no heterogeneous phase and having high crystallinity can be prepared at a low cost.

[0082] In addition, the steps of this embodiment are simple, and it is therefore easy to increases manufacturing efficiency by conducting the steps successively. The method of the present invention makes it possible to mass-produce a high quality BaTiO₃ powder at a low cost.

[0083] The method of the present invention is not limited to the above-described embodiment. In the above embodiment, Ba(OH)₂.8H₂O is fused and dissolved by heating to prepare a solution of a high concentration of Ba. However, barium hydroxide anhydride (Ba(OH)₂) may be mixed with water in an amount equivalent to the amount of the crystal water contained in Ba(OH)₂.8H₂O to prepare the solution of a high concentration of Ba. Thus, a fine BaTiO₃ powder having high crystallinity may be prepared, as in the earlier described embodiment.

[0084] Here, the BaTiO₃ reaction product is yielded in a slurry form by the reaction of the Ba solution with the TiO₂ in the reaction step 1b. The reaction product BaTiO₃ may be further exposed to ultrasonic waves having a frequency of about 10 to 30 kHz while being stirred. By applying the ultrasonic waves, much finer cubic crystalline BaTiO₃ having a specific surface area Sw of about 60 to 100 m²/g and containing no heterogeneous phase can be prepared before calcination.

[0085] The foregoing has described a method applied to the preparation of BaTiO₃ powder in detail. However, the method can be applied to the preparation of other complex oxides having a perovskite structure, such as SrTiO₃ and (Ba, Ca)TiO₃.

EXAMPLES

[0086] Examples of the present invention will now be described.

Experiment 1

[0087] The inventors first investigated the reaction path of BaTiO₃ synthesis.

[0088] Anatase-type TiO₂ having a specific surface area Sw of 330 m²/g and Ba(OH)₂.8H₂O were weighed such that the mole ratio of Ba to Ti in the BaTiO₃ to be synthesized is 1. Specifically, 57.342 g of TiO₂ and 202.88 g of Ba(OH)₂.8H₂O were weighed. They were placed in a container heated to 70° C. and allowed to react, and the process of BaTiO₃ production was observed.

[0089] FIGS. 4 to 6 are transmission electron micrographs of crystals in the process of BaTiO₃ synthesis.

[0090]FIG. 4 shows crystals after 5 minutes have elapsed from the start of the reaction, taken at a magnification of 790,000 times by transmission electron microscopy (TEM). FIGS. 5 and 6 show crystals in the region surrounded by the circle shown in FIG. 4 after 30 and 60 minutes have elapsed from the start of the reaction, taken at a magnification of 390,000 times by TEM.

[0091] FIGS. 4 to 6 suggest that TiO₂ powder initially having a particle size of about 5 nm grows to BaTiO₃ having a particle size of about 20 nm while the reaction proceeds.

[0092] The mole ratio Ba/Ti was measured by energy dispersive X-ray spectroscopy (EDX). As a result, the mole ratio Ba/Ti was 6/29 after 5 minutes had elapsed from the start of the reaction (FIG. 4), and it changed to 19/20 after 30 minutes had elapsed from the start of the reaction (FIG. 5), showing that the Ba and Ti molar contents were substantially the same.

[0093] The reaction generally proceeds through the two reaction paths shown in FIG. 2 (reaction path 1) and FIG. 3 (reaction path 2). However, the particles in the series of the reaction shown in FIGS. 4 to 6 in this example were single crystals and did not exhibit diffusion of part of the Ba. Therefore, it is concluded that the reaction proceeded through reaction path (1).

Experiment 2

[0094] A BaTiO₃ reaction product prepared as in Example 1 was placed in a desk-top sand mill with 800 g of partially stabilized zirconia (PSZ) of 1 mm in diameter serving as pulverizing media, and was agitated and pulverized at 70° C. for 1 hour at a rotation speed of 9 s⁻¹ (540 rpm) to prepare a slurry. The slurry taken out from the mill was dried at 200° C. in an oven to form a solid. The solid was divided into three portions, and each solid was calcined at 900, 950 or 1000° C. to yield BaTiO₃ powder of Example 1. The mole ratio Ba/Ti of Ba to Ti of the resulting BaTiO₃ powder was 0.998, according to X-ray fluorescence analysis (XRF).

[0095] The specific surface areas Sw of the BaTiO₃ powders of Example 1, prepared at different calcination temperatures, were measured by the Brunauer-Emmett-Teller (BET) method and the equivalent specific surface diameters D were derived from the specific surface areas. The powders of Example 1 were subjected to powder X-ray diffraction (XRD), and the axial ratio c/a of the c axis to the a axis of the crystals was calculated based on the XRD results. For the sake of comparison, non-calcined powder dried at 200° C. was also subjected to the same measurement.

[0096] Table 1 shows the results. TABLE 1 Equivalent Calcination Specific specific surface Temperature Mole ratio Axial ratio surface area Sw diameter D (° C.) A site/B site c/a (m²/g) (nm) non-calcined 0.998 1.0000 47.61 21.0 (dried at 200° C.) 900 0.998 1.0075 7.31 137 950 0.998 1.0082 5.69 176 1000 0.998 1.0088 3.88 258

[0097] As shown in Table 1, the non-calcined powder exhibited a specific surface area Sw of 47.61 m²/g, a small equivalent specific surface diameter D of 21.0 nm, and a axial ratio c/a of 1.000, indicating a cubic system.

[0098] Table 1 also suggests that the particle size is increased by calcination and that, as the particle size becomes larger, the axial ratio c/a increases so that the crystal system changes from a cubic system to a tetragonal system.

[0099] FIGS. 7 to 10 are scanning electron micrographs of the non-calcined powder and powders of Example 1 calcined at 900, 950 or 100°C. They show that, as the calcination temperature becomes higher, the particles grow to be larger.

[0100]FIG. 11 shows the results of XRD. The horizontal axis represents the diffraction angle 2θ and the vertical axis represents intensity (arbitrary unit). In FIG. 11, the white triangles represent BaCO₃ which could be by-produced in the reaction, and the black squares represent Ba₂TiO₄ having a Ba content higher than that of BaTiO₃.

[0101] As shown in FIG. 11, even the non-calcined powder exhibits a peak of cubic crystalline BaTiO₃. It is therefore shown that cubic crystalline BaTiO3 having high crystallinity can be produced even by synthesis at a low temperature of 70° C., and that heterogeneous phases, such as BaCO₃ and Ba₂TiO₄, are hardly by-produced.

[0102] Thus, ultrafine, cubic crystalline BaTiO₃ having high crystallinity can be produced before calcination, as distinct from the known methods such as the pulverization method. Therefore, ultrafine, tetragonal crystalline BaTiO₃ powder can be obtained by calcination.

[0103] BaTiO₃ powders of Comparative Examples 1 and 2 were prepared by the hydrothermal synthesis and the alkoxide-hydroxide route, respectively. The relationship between the particle size and the axial ratio c/a of the BaTiO₃ powders of Example 1 and Comparative Examples 1 and 2 were investigated.

[0104] The BaTiO₃ powder of Comparative Example 1 was prepared by the following procedure.

[0105] In 10 mL of water, 0.01 mol of NaOH was dissolved to prepare a NaOH solution, and 2.5 mL of BaCl₂ or Ba(OH)₂ and 2.5 mL of TiO₂ were added to the NaOH solution. The mixture was heated in an autoclave to react under conditions of a high temperature of 250° C. and a high pressure of 5 MPa. The resulting precipitate was filtered and washed with water.

[0106] The reaction product was subjected to XRD and unreacted TiO₂ and BaCO₃ were not detected.

[0107] The reaction product was allowed to react with BaCl₂ for one week to prepare a tetragonal crystalline BaTiO₃ having a particle size of 50 nm. Then, the BaTiO₃ was divided into three portions, and each was calcined at 900, 950 or 1000° C. to yield a BaTiO₃ powder of Comparative Example 1.

[0108] The BaTiO₃ powder of Comparative Example 2 was prepared by the following procedure.

[0109] Into a solution of 2.5×10³ mol/m³ titanium isopropoxide (Ti[OCH(CH₃)₂]₄) maintained at a temperature of 60° C., Ba(OH)₂.8H₂O powder was added such that the mole ratio Ba/Ti of Ba to Ti of BaTiO₃ to be synthesized is 1, and was strongly stirred. After the Ba(OH)₂ was uniformly dissolved and then 3 minutes elapsed, the solution became clouded and gelled. The resulting gelled slurry was subjected to infrared spectroscopy. As a result, absorption bands were observed at 380 cm ⁻¹ and 570 cm⁻¹; hence, it was shown that a substance having a perovskite structure was present in the gelled slurry.

[0110] The gelled slurry was dried in an oven heated to 150° C. for 2 hours to yield a BaTiO₃ powder having a particle size of 48 nm. This BaTiO₃ powder had a mole ratio Ba/Ti of 0.998 and a specific surface area Sw of 45 m²/g, according to XRF. The BaTiO₃ powder was divided into three parts, and each was calcined at 900, 950 or 1000° C. to yield BaTiO₃ powder of Comparative Example 2.

[0111]FIG. 12 shows the relationship between the particle size and the axial ratio of the calcined BaTiO₃ of Example 1 and Comparative Examples 1 and 2. The white circles, black rhombus, and white squares shown in FIG. 12 represent Example 1, Comparative Example 1 and Comparative Example 2, respectively.

[0112]FIG. 12 shows that BaTiO₃ of Example 1 has an larger axial ratio c/a and a smaller particle size than those of Comparative Example 1, a cubic system having high crystallinity.

[0113] The BaTiO₃ of Comparative Example 2 by the alkoxide-hydroxide route had crystallinity higher than that of Example 1. However, the alkoxide-hydroxide route needs a molar amount of Ba(OH)₂ which was 2 to 3 times larger than that of TiO₂, and thus needs such an excessive amount of Ba(OH)₂.

[0114] In contrast, the molar amounts of TiO₂ and Ba(OH)₂ used in Example 1 are substantially the same. It is not necessary to use an excessive amount of Ba(OH)₂, and therefore Ba²⁺ does not remain in the solution after the synthesis. Thus, it is easy to control the composition of BaTiO₃ and to reduce manufacturing costs.

[0115] Experiment 3

[0116] BaTiO₃ powders were prepared using TiO₂ powders having different specific surface areas Sw according to the following procedure, and subjected to XRD to investigate whether a heterogeneous phase was present.

[0117] Anatase-type TiO₂ powder having a specific surface area of 250 m²/g in an amount of 62.410 g and Ba(OH)₂.8H₂O in an amount of 119.77 g were weighed so that the mole ratio Ba/Ti of Ba to Ti of BaTiO₃ to be synthesized would be 1.

[0118] The weighed materials were placed in a desk-top sand mill with 800 g of PSZ of 1 mm in diameter and agitated and pulverized at 70° C. for 1 hour at a rotation speed of 9 s⁻¹ (540 rpm) to prepare a slurry, as in Experiment 2. The slurry taken out from the mill was dried at 200° C. in an oven to yield BaTiO₃ of Example 11 in a solid form.

[0119] In the same manner, anatase-type TiO₂ powder having a specific surface area of 300 m²/g in an amount of 189.28 g and Ba(OH)₂.8H₂O in an amount of 56.898 g were weighed so that the mole ratio Ba/Ti of Ba to Ti of BaTiO₃ to be synthesized would be 1. Thus, BaTiO₃ of Example 12 was prepared in a solid form, as in Example 11.

[0120] In the same manner, anatase-type TiO₂ powder having a specific surface area of 330 m²/g in an amount of 202.01 g and Ba(OH)₂.8H₂O in an amount of 56.898 g were weighed so that the mole ratio Ba/Ti of Ba to Ti of BaTiO₃ to be synthesized would be 1. Thus, BaTiO₃ of Example 13 was prepared in a solid form, as in Example 11.

[0121] Furthermore, in the same manner, anatase-type TiO₂ powder having a specific surface area of 240 m²/g in an amount of 75.721 g and Ba(OH)₂.8H₂O in an amount of 270.51 g were weighed so that the mole ratio Ba/Ti of Ba to Ti of BaTiO₃ to be synthesized would be 1. Thus, BaTiO₃ of Comparative Example 11 was prepared in a solid form, as in Example 11.

[0122] The BaTiO₃ of Examples 11 to 13 and Comparative Example 11 were subjected to XRD.

[0123]FIG. 13 shows the results of XRD. The horizontal axis represents the diffraction angle 2θ and the vertical axis represents intensity (arbitrary unit). The white triangles, black squares and white squares represent heterogeneous phases of BaCO₃, Ba₂TiO₄ and BaTi₂O₅, respectively. For example, Comparative Example 11 exhibits two sharp peaks at diffraction angles 2θ of 25° and 28° with white squares thereabove, which show the formation of heterogeneous phases of BaTi₂O₅. Comparative Example 11 also exhibits a sharp peak at a diffraction angle 2θ of 29° with a black square thereabove, which shows the formation of a heterogeneous phase of Ba₂TiO₄.

[0124] As shown in FIG. 13, while the BaTiO₃ of Example 11 (specific surface area Sw: 240 m²/g) includes heterogeneous phases of BaCO₃, BaTi₂O₅ and Ba₂TiO₄ between a wide rage of diffraction angles 2θ of 20° to 60°, the Examples 11 to 13 (specific surface areas Sw: 250 to 330 m²/g) include few heterogeneous phases of BaCO₃ and no BaTi₂O₅ or Ba₂TiO₄. Thus, it is shown that TiO₂ powder must have a specific surface area of at least about 250 m²/g.

[0125] Experiment 4

[0126] The BaTiO₃ reaction product slurry was exposed to ultrasonic waves, and properties of the resulting powder was investigated.

[0127] First, 150 mL of water was placed in a vessel heated by circulating vapor of 100° C. to prepare hot water of 60° C. Anatase-type TiO₂ having a specific surface area of 300 m²/g in an amount of 98.067 g and Ba(OH)₂ in an amount of 185.318 g were weighed so that the mole ratio Bi/Ti of Ba to Ti of BaTiO₃ to be synthesized would be 1.003, and were then added to the hot water. The Ba(OH)₂ was allowed to start reacting, with heat generated, to prepare BaTiO₃ in a slurry form.

[0128] The BaTiO₃ was stirred with a magnetic stirrer while being exposed to ultrasonic waves having a frequency of 16 kHz by immersing in the horn of an ultrasonic emitter.

[0129] Then, the BaTiO₃ was pulverized with a desk-top sand mill, in substantially the same manner as Experiment 2, to prepare a slurry. The slurry was taken out of the mill and placed in an oven heated to 200° C. to dry. Thus, a non-calcined solid BaTiO₃ was prepared.

[0130] The mole ratio Ba/Ti of Ba to Ti of the resulting non-calcined BaTiO₃ was 0.9998, according to XRF analysis.

[0131] The non-calcined BaTiO₃ was subjected to XRD to investigate whether a heterogeneous phase was present.

[0132]FIG. 14 shows the results of XRD. The horizontal axis represents the diffraction angle 2θ and the vertical axis represents intensity (arbitrary unit).

[0133] As shown FIG. 14, the non-calcined BaTiO₃ does not include any heterogeneous phases such as Ba₂TiO₄, and it is therefore shown that a pure, solid BaTiO₃ can be prepared before calcination.

[0134] The axial ratio c/a of the non-calcined solid BaTiO₃ was calculated from the results of XRD, as in Experiment 2. Also, the specific surface area Sw of the BaTiO₃ was measured by the BET method and the equivalent specific surface diameter D was derived from the specific surface area Sw.

[0135] Table 2 shows the results. TABLE 2 Equivalent Specific specific surface Mole ratio Axial ratio surface area diameter D A site/B site c/a Sw (m²/g) (nm) BaTiO₃ 0.9998 1.0000 64.08 15.6 dried at 200° C.

[0136] Table 2 shows that the non-calcined BaTiO₃ dried at 200° C. after exposure of ultrasonic waves has a specific surface area Sw of 64.08 m²/g and an equivalent specific surface diameter D of 15.6 nm, smaller than that of the non-calcined BaTiO₃ in Experiment 2, shown in Table 1. It is therefore shown that the exposure to ultrasonic waves contributes to the reduction of the particle size of BaTiO₃. Also, the axial ratio c/a is 1.000, showing a cubic system.

[0137] Experiment 5

[0138] A BaTiO₃ dried in an oven heated to 200° C., as in Experiment 2, was placed in a ball mill with isopropyl alcohol, and was wet-pulverized for 10 hours to be dispersed in the isopropyl alcohol. The dispersed BaTiO₃ was dried at 200° C. in an oven to form a solid. The solid was divided into three portions, and each solid was calcined at 900, 950 or 1000° C. for 2 hours to yield a calcined BaTiO₃ powder.

[0139] The axial ratio c/a, the specific surface area Sw, and the equivalent specific surface diameter D of the resulting calcined BaTiO₃ powders and the non-calcined BaTiO₃ at dried at 200° C. were measured.

[0140] Table 3 shows the results. TABLE 3 Equivalent Calcination Axial specific specific surface Temperature Mole ratio ratio surface area diameter D (° C.) A site/B site c/a Sw (m²/g) (nm) non-c alcined 0.998 1.0000 55.2 18.1 (dried at 200° C.) 900 0.998 1.0080 7.53 133 950 0.998 1.0092 4.90 204 1000 0.998 1.0098 3.25 308

[0141] Table 3 shows that by calcining at a temperature of 950° C. or more, the specific Sw is reduced, but the axial ratio c/a can be increased in comparison with experiment 2, shown in Table 1, in which the dispersion step was not performed. 

What is claimed is:
 1. A method for preparing a complex oxide powder having a perovskite structure expressed by the general formula ABO₃, the method comprising dissolving a hydroxide of an element constituting the A site of the general formula ABO₃ in water to form a fused hydroxide; and allowing the fused hydroxide to react with an oxide powder of an element constituting the B site of the general formula ABO₃ to form a reaction product comprising the oxide powder in the form of ultrafine particles.
 2. A method for preparing a complex oxide powder according to claim 1, wherein the hydroxide contains water of hydration and the hydroxide is dissolved in the water of hydration by heating.
 3. A method for preparing a complex oxide powder according to claim 2, wherein the hydroxide is barium hydroxide octahydrate and the oxide powder of the B site element is titanium oxide powder.
 4. A method for preparing a complex oxide powder according to claim 3, wherein particles of the oxide powder of the B site element have a specific surface area of about 250 m²/g or more.
 5. A method for preparing a complex oxide powder according to claim 4, wherein the reaction further comprises ultrasonication.
 6. A method for preparing a complex oxide powder according to claim 6, further comprising calcining the reaction product.
 7. A method for preparing a complex oxide powder according to claim 1, wherein the fusion product is formed by dissolving an anhydrous hydroxide of an element constituting the A site of the general formula ABO₃ in water.
 8. A method for preparing a complex oxide powder according to claim 7, wherein the amount of water is about the same as the amount of water of hydration contained in a hydrous hydroxide of the element constituting the A site.
 9. A method for preparing a complex oxide powder according to claim 8, wherein the anhydrous hydroxide is barium hydroxide anhydride and the oxide powder of the B site element is titanium oxide powder.
 10. A method for preparing a complex oxide powder according to claim 9, wherein the particles of the oxide powder of the B site element ave a specific surface area of 250 m²/g or more.
 11. A method for preparing a complex oxide powder according to claim 10, wherein the reaction further comprises ultrasonication.
 12. A method for preparing a complex oxide powder according to claim 12, further comprising calcining the reaction product.
 13. A method for preparing a complex oxide powder according to claim 1, wherein the hydroxide and the oxide powder are weighed such that the mole ratio of the A-site element A to the B-site element B is in the range of about 0.990 to 1.010.
 14. A method for preparing a complex oxide powder according to claim 1, wherein the reaction is performed under atmospheric pressure.
 15. A method for preparing a complex oxide powder according to claim 1, wherein the reaction further comprises ultrasonication.
 16. A method for preparing a complex oxide powder according to claim 15, wherein the reaction product has a specific surface area in the range of about 60 to 100 m²/g.
 17. A method for preparing a complex oxide powder according to claim 1, further comprising calcining the reaction product.
 18. A method for preparing a complex oxide powder according to claim 1, further comprising dispersing the reaction product in a liquid; and calcining the dispersed reaction product.
 19. A method for preparing a complex oxide powder according to claim 1, wherein the oxide of the B site element is anatase TiO₂.
 20. A complex oxide powder prepared by the method for preparing a complex oxide powder according to claim
 1. 